Your SlideShare is downloading. ×
0
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Chapter #2   Lecture Part 2
Upcoming SlideShare
Loading in...5
×

Thanks for flagging this SlideShare!

Oops! An error has occurred.

×
Saving this for later? Get the SlideShare app to save on your phone or tablet. Read anywhere, anytime – even offline.
Text the download link to your phone
Standard text messaging rates apply

Chapter #2 Lecture Part 2

478

Published on

Published in: Education, Technology
0 Comments
1 Like
Statistics
Notes
  • Be the first to comment

No Downloads
Views
Total Views
478
On Slideshare
0
From Embeds
0
Number of Embeds
0
Actions
Shares
0
Downloads
16
Comments
0
Likes
1
Embeds 0
No embeds

Report content
Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

Cancel
No notes for slide
  • Figure 2.13
  • Transcript

    • 1. Atomic Mass
      • Atomic and molecular masses can be measured with great accuracy with a mass spectrometer.
    • 2. Average Atomic Mass or Atomic Weight
      • Because in the real world we use large amounts of atoms and molecules, we use average masses in calculations.
      • Average mass is calculated from the isotopes of an element weighted by their relative abundances.
    • 3. Periodic Table
      • A systematic catalog of elements.
    • 4. Periodicity
      • When one looks at the chemical properties of elements, one notices a repeating pattern of reactivities.
    • 5. Periodic Table
      • The rows on the periodic chart are periods.
    • 6. Groups
    • 7. Periodic Table
      • Nonmetals are on the right side of the periodic table (with the exception of H).
    • 8. Periodic Table
      • Metalloids border the stair-step line (with the exception of Al and Po).
    • 9. Periodic Table
      • Metals are on the left side of the chart.
    • 10. Chemical Formulas
      • The subscript to the right of the symbol of an element tells the number of atoms of that element in one molecule of the compound.
    • 11. Molecular Compounds
      • Molecular compounds are composed of molecules and almost always contain only nonmetals.
    • 12. Diatomic Molecules
      • These seven elements occur naturally as molecules containing two atoms.
    • 13. Types of Formulas
      • Empirical formulas give the lowest whole-number ratio of atoms of each element in a compound.
      • Molecular formulas give the exact number of atoms of each element in a compound.
    • 14. Types of Formulas
      • Structural formulas show the order in which atoms are bonded.
      • Perspective drawings also show the three-dimensional array of atoms in a compound.
    • 15. Ions
      • When atoms lose or gain electrons, they become ions.
        • Cations are positive and are formed by elements on the left side of the periodic chart.
        • Anions are negative and are formed by elements on the right side of the periodic chart.
    • 16. Ionic Bonds
      • Ionic compounds (such as NaCl) are generally formed between metals and nonmetals.

    ×